Example Of A Displacement Reaction

Reactivity series

The reactivity series allows us to predict how metals will react. A more than reactive metal will displace a less reactive metallic from a compound. Rusting is an oxidation reaction.

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Deportation reactions of solutions

A more reactive metallic will displace a less reactive metallic from a solution of one of its salts. For example:

magnesium + copper(2) sulfate → copper + magnesium sulfate

Mg(s) + CuSO ₄ (aq) → Cu(s) + MgSO _iv (aq)

In this reaction, the blue colour of the copper(II) sulfate fades equally it is used up (magnesium sulfate solution is colourless). We would likewise see copper metal forming.

Reactions between metals and solutions of metal salts allow usa to put a selection of metals into a reactivity series. Using metals J, Yard and L:

	Metal J	Metal K	Metal L
J sulfate	X	No reaction	No reaction
K sulfate	Displaces K	X	Displaces M
50 sulfate	Displaces L	No reaction	X

Metal J displaces both Thousand and Fifty - so it must be the virtually reactive and exist at the summit of this reactivity series.

Metal K cannot displace either J or L - so it must be the least reactive and exist at the lesser of this reactivity series.

Metal L displaces K only cannot displace J - so it must be more reactive than K but less reactive than J, and be in between them in this reactivity serial.

Therefore, the society is:

A list of letters from most reactive to least reactive: J, L and K.

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